Question

An aqueous solution containing a substance whose concentration is 7.50 g/L has an osmotic pressure of 1150 Torr at 77 K.

(a) What is the molecular weight of the solute?

(b) What is the osmotic pressure of a solution at 27 degrees C that contains 1.00 g of this solute in 500 mL of solution?

Answer #1

PV = nRT

P = 1150torr = 1150/760 = 1.513atm

W = 7.5g

V = 1L

T = 77K

PV = WRT/M

M = WRT/PV

= 7.5*0.0821*77/1.513*1 = 31.34g/mole

b. PV = nRT

PV = WRT/M

W = 1g

M = 31.34g/mole

T = 27C = 27+273 = 300K

V = 500ml = 0.5L

PV = WRT/M

P = WRT/VM

= 1*0.0821*300/0.5*31.34 = 1.57atm

1. A solution of 7.50 mg of a small protein in 5.00 mL aqueous
solution has an osmotic pressure of 5.05 torr at 23.1 degrees
celcius. What is the molar mass of the protein?
2. A 179 mg sample of a nonelectrolyte isolated from throat
lozenges was dissolved in enough water to make 10.0 mL of solution
at 25 degrees celcius. The osmotic pressure of the resulting
solution was 4.81 atm. Calculate the molar mass of the
compound.

A b
and c are containers containing respectively 10 g NACl in 50 ml
aqueous solution, 0.20 mol NACl
in 100
mL of aqueous solution and 500 mL of aqueous MgCl2 solution whose
concentration is 1 mol / L. (Data: M (NA) = 23 g / mol; M (Mg) =
24.3 g / mol; M (Cl) = 35.5 g / mol) Mixing the three solutions
determine the concentrations in mol / L of NaCl and MgCl2

In a laboratory experiment, a student found that a
158-mL aqueous solution containing
2.589 g of a compound had an osmotic pressure of
13.5 mm Hg at 298 K. The compound
was also found to be nonvolatile and a nonelectrolyte. What is the
molar mass of this compound?
The nonvolatile, nonelectrolyte aspirin,
C9H8O4
(180.1 g/mol), is soluble in
chloroform
CHCl3.
Calculate the osmotic pressure (in atm) generated when
14.4 grams of aspirin are
dissolved in 185 mL of a
chloroform...

The osmotic pressure of 100.0 mL of a 25 C solution containing
0.50 g of a protein is 5.8 Torr. Based on this information,
determine the molar mass of the protein in g/mol.
Hint: The protein does not dissociate in water;
thus the Van't Hoff factor equals 1.
a) 1.6 x 101
b) 1.6 x 103
c) 1.6 x 104

1a.) Calculate the osmotic pressure of a solution that contains
95.0 g of the nonelectrolyte urea, CH4N2O,
per 500 mL of solution at 25°C.
a.) 75.4 atm,
b.) 69.8 atm,
c.) 84.4 atm,
d.) 77.4 atm
1b.) Calculate the osmotic pressure of a 0.060M glucose solution
at 27°C.
a.) 3.4 atm,
b.) 1.2 atm,
c.) 5.8 atm,
d.) 1.5 atm
PLEASE CIRCLE THE ANSWERS.

What is the vapor pressure of an aqueous solution containing 10
%(by weight) ethylene glycol (62 g/mol) at 25 C. PH2O= 24.3 torr at
25 C.

When 2.38 g of a nonelectrolyte solute is dissolved in water to
make 705 mL of solution at 27 °C, the solution exerts an osmotic
pressure of 801 torr.
A) What is the molar concentration of the solution?
B) How many moles of solute are in the solution?
C) What is the molar mass of the solute?

When 2.56 g of a nonelectrolyte solute is dissolved in water to
make 825 mL of solution at 24 degrees Celcius, the solution exerts
an osmotic pressure of 887 torr.
A) What is the molar concentration of the solution?
B) How many moles of solute are in the solution?
C) What is the molar mass of the solute in g/mol?

What is the osmotic pressure of a solution of 12.5 g sucrose
(C12H22O11) in 225 g water at 50.0 °C? Assume that the density of
the solution is 1.00 g/mL

Calculate the osmotic pressure of a magnesium citrate laxative
solution containing 28.0 g of magnesium citrate in 225 mL of
solution at 37 ∘C (approximate body temperature). Assume complete
dissociation of the ionic compound.

ADVERTISEMENT

Get Answers For Free

Most questions answered within 1 hours.

ADVERTISEMENT

asked 6 minutes ago

asked 12 minutes ago

asked 18 minutes ago

asked 23 minutes ago

asked 29 minutes ago

asked 29 minutes ago

asked 36 minutes ago

asked 36 minutes ago

asked 36 minutes ago

asked 50 minutes ago

asked 1 hour ago

asked 1 hour ago